(Original post by A Sajid)
Low temperatures push the reaction to the exothermic side. And the forward reaction/ product had less molecules than the reactants. So increase in pressure pushed the equilibrium to the product side. And then you talk about how high pressure costly blah blah.

But if low temp and high pressure push the equilibrium to the product/right hand side then surely that wouldn't produce a good percentage yield since more of the product would break down to form reactants?? There was a similar question in one of the specimen depth papers which is had a contradictory answer to the question in today's paper?

(Original post by Jitesh)
Certainly but not sure how many with it being a new spec and all